kinetic theory of gases Flashcards
1st 3 ideas of kinetic theory
particles move in continuous, random straight line motion
average distance between gas particles is large compared to size of particles
negligible intermolecular forces between gas particles
2nd 3 main ideas of kinetic theory
collisions between gas particles are elastic
pressure is caused when gas particles hit the walls of their container
temperature is a measure of the average KE of particles
compressibility
the ability to decrease the distance between particles
average distance between the gas particles is very large compared to the size of the particles themselves, so you can compress the gas by reducing distance between it.
diffusion
diffusion is the movement of particles from an area of high conc to low conc
odours can be smelt from far away
particles of gases will move in random straight line motion, causing them to spread from areas of high conc to areas of low conc + fill container
ideal gas
imaginary gas which always follows principles of kinetic theory of gases
- large distance between particles
- no attraction between particles
real gases
will deviate from these trends, particularly at very low temperatures
- distances between particles gets smaller
- attraction (IM forces) between particles gets stronger
tempearture and pressure
proportional
the higher the temperature, the higher the KE, the faster the particles are moving, so the more collisions of particles on the outside of the container, so higher pressure
temperature and volume
proportional
the higher the temperature of the particles, the higher the KE, the faster and more the particles move, the more space it takes up, the higher the volume.
pressure and volume
inversely proportional
when container is made smaller, it compresses the gas and the particles collide with the container sides more so higher pressure with lower volume
